A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl2(9)+2e + 2 C1¯(aq) =+1.359 V red N2(9)+4 H2O(1)+4e N2H4(aq)+4 OH (aq) E=-1.16 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that | happens at the cathode. Write a balanced equation for the half-reaction that U happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl2(9)+2e + 2 C1¯(aq) =+1.359 V red N2(9)+4 H2O(1)+4e N2H4(aq)+4 OH (aq) E=-1.16 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that | happens at the cathode. Write a balanced equation for the half-reaction that U happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A galvanic cell is powered by the following redox reaction: 3 Br₂(1) + 2NO(g) + 4H₂O(1) - 6 Br (aq) + 2NO3(aq) + 8H (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 E = v 00 Ś
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Cro (aq) + 4 H₂O(1)+3e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is swer the following questions about this cell. spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? 2+ Cu (aq) + e If you said it was possible to calculate the cell voltage, do so and enter your answer 0 half-reaction 0 2 Cu²+ (aq) + e → Cu (aq) Yes No + 0.28 V Cu (aq) Cr(OH)3(s)+5 OH (aq) standard reduction potential E .0 'red Eº ´red = +0.153 V -0.13 V ロ→ロ e × x10 Ś
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Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and Cl₂ (g), when the two are brought in contact via standard half-cells in a voltaic cell. Cl₂(g) + 2e → 2Cl(aq) = 1.360 V red = -0.280 V Co²+ (aq) + 2e → Co(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
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